Answer:
P(total) = 1110 mmHg
Explanation:
According to the Dalton law of partial pressure,
The pressure exerted by mixture of gases are equal to the sum of partial pressure of individual gases.
P(total) = P1 + P2 + P3+ .....+ Pn
Given data:
Sample A = 740 mmHg
Sample B = 740 mmHg
Sample C = 740 mmHg
Total pressure = ?
Solution:
<em>Sample A:</em>
P₁V₁ = P₂V₂
P₂ = P₁V₁ / V₂
P₂ = 740 mmHg × 2L/4L
P₂ = 370 mmHg
<em>Sample B:</em>
P₁V₁ = P₂V₂
P₂ = P₁V₁ / V₂
P₂ = 740 mmHg × 2L/4L
P₂ = 370 mmHg
<em>Sample C:</em>
P₁V₁ = P₂V₂
P₂ = P₁V₁ / V₂
P₂ = 740 mmHg × 2L/4L
P₂ = 370 mmHg
Total pressure:
P(total) = P1 + P2 + P3
P(total) = 370 mmHg + 370 mmHg+ 370 mmHg
P(total) = 1110 mmHg
Ideal gas is defined as hypothetical gas that fits all the assumptions of the kinetic-molecular theory. There are several assumption statement that apply to the behavior of an ideal gas, First Gases consist of larger number of tiny particles that are far apart relative to their size, Second, collisions between gas particles and between particles and container walls are elastic collision, third, gas particles are in rapid, random motion and continuous, Fourth, the temperature of a gas depends on the average kinetic energy of the particles of the gas.
<span>An organism that contains chloroplasts is able to produce food by the process of
"Photosynthesis"
Hope this helps!
</span>
Answer:
Molar mass of KClO₃ = (39 + 35.5 + 16×3) g/mol = 122.5 g/mol
Molar mass of KCl = (39 + 35.5) g/mol = 74.5 g/mol
Balanced equation for the reaction:
2KClO₃ → 2KCl + 3O₂
Mole ratio KClO₃ : KCl = 2 : 2
Moles of KClO₃ reacted = (2.73 g) / (122.5 g/mol) = 0.0223 mol
Moles of KCl formed = (0.0223 mol) × (2/2) = 0.02229 mol
Mass of KCl formed = (0.0223 mol) × (74.5 g) = 1.66 g
====
OR:
(2.73 g KClO₃) × (1 mol KClO₃ / 122.5 g KClO₃) × (2 mol KCl produced / 2 mol KClO₃) × (74.5 g KCl / 1 mol KCl)
= 1.66 g KCl produced